chapter 6 part 1

light is

electromagnetic radiation

light is characterized by:

wavelength and frequency

Wavelength (λ)

the distance between 2 points on a wave

wavelength units

meters or nanometers

frequency (V)

a measure of the number of wave cycles that move through a point in space in 1 second

frequency units 

hertz (Hx)

electromagnetic spectrum

the entire range of electromagnetic radiation

as wavelength increase, frequency and energy of light will? 

frequency and energy of light decreases

threshold frequency

a phenomenon in which electrons are ejected from the surface of certain metals exposed to light of at least a certain minimum frequency

photons

packets of lights

light exists as

waves and particles

wave equation

c = λν

c is speed of light 

E_photon =

hv= hc/λ

longer wavelength =

smaller photon energy

Niels Bohr studied 

the line spectra of the hydrogen atom to understand the e^-

Bohr created the

planetary model

Bohr’s planetary model was based on the idea

that e^- and their energies can only have certain values

ground state

the lowest energy level closest the the nucleus

excited states 

absorption spectrum is observed when e^-  absorb energy and move to higher states 

ΔE =

E_final − E_initial

E_photon 

|ΔE|

rydberg equation =

1/λ (R_h=1.097 × 10⁷ m^-1 ) (1/n₁²) (1/n₂²)

the s subshell contains how many orbitals 

1 orbital 

the p subshell contains how many orbitals 

3 orbitals

the d subshell contains how many orbitals 

5 orbitals

the f subshell contains how many orbitals 

7 orbitals

subshells from lowest to highest energy 

s - p - d- f

what sublevels are in the principal energy level n=1?

single s sublevel 

what sublevels are in the principal energy level n=2?

s and p sublevel, 2s and 2p sublevel (three 2p orbitals)

what sublevels are in the principal energy level n=3?

s,p,d - 3s, 3p (3 orbitals), and 3d (5 orbitals )

what sublevels are in the principal energy level n=4?

s,p,d,f - 4s, 4p (3 orbitals) , 4d (5 orbitals) , and 4f orbitals (7 orbitals)

principal quantum #

n, values are postive integers starting with 1

angular quantum number

ℓ, identifies the sublevel or subshell of electron

allowed values for ℓ

0 to (n-1)

angular quantum #: ℓ = 0, subshell = ?

subshell s

angular quantum #: ℓ = 1, subshell = ?

subshell p

angular quantum #: ℓ = 2 subshell = ?

subshell d

angular quantum #: ℓ = 3 subshell = ?

subshell f

magnetic quantum number

mℓ , identifies the orbital that the e^- occupies 

allowed values for mℓ

-ℓ to +ℓ

spin quantum number

m_s , corresponds to the specific electron in orbial a

allowed values for m_s

+1/2 or -1/2

orbital diagrams 

graphical representation that show the sublevels and orbitals at each principal level 

degnerate

orbitals within a subshell are the same energy level

pauli-exclusion principle

max 2 electrons can occupy each orbital

aufbau principle

electrons fill orbitals with the lowest energy orbital

hund’s rule 

Electrons are distributed into orbitals of identical energy (same sublevel) in such a way as to give the maximum number of unpaired electrons.

paramagnetic

at least one unpaired e^-

diamagnetic

no unpaired e^-